Question

Identify the Bronsted acids and bases in the following equation (multiple choice)

Answer 1

Reactions according to Bronsted are those in which there is an exchange of H+ ions. The Bronsted acid will be the substance that donates H+ ions and the base will be the compound that receives them.

As a result we will have a conjugated acid and a conjugated base. The conjugate acid will be the former base that just received the H+ ions. The conjugate base will be the former acid that donated its H+ ions.

Now let's look at the reaction. On the reactants side the compound that can donate H+ ions will be HSO3- and the compound CN- will be the one that receives them. Therefore, HSO3 will be the Bronsted acid (A) and CN will be the base (B).

HSO3 ---> A

CN -----> B

Now let's look at the product side. The compound that received the H+ ions will be the compound HCN, so this will be the conjugate acid (Ac). And the compound that lost its H+ ions is SO3, so it will be the conjugate base (Bc).

HCN --->Ac

SO3 ---->Bc

Comparing the analysis that we did with the reaction we will have that:

`\begin{gathered} HS_{}O^-_3+CN^-\rightleftarrows HCN+SO^(2-)_3 \\ A+B\rightleftarrows Ac+Bc \end{gathered}`

So, the answer will be option number 5